That element is a member of the Actinides (it's probably one of the following: Ac, Th, Pa, U, Np, Cm, Bk, Lr)
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
Lanthanide or Actinide
The s sublevel has just one orbital, so can contain 2 electrons max. The p sublevel has 3 orbitals, so can contain 6 electrons max. The d sublevel has5orbitals, so can contain 10 electrons max. And the 4 sublevel has 7 orbitals, so can contain 14 electrons max.
The d sublevel has 5 orbitals, and each orbital can contain a maximum of 2 electrons, so the d sublevel can hold a maximum of 10 electrons.
The 4f sublevel has 7 orbitals, each of which can contain 2 electrons. So the maximum number of electrons in the 4f sublevel is 14.
Tungsten atoms contain six energy levels (shells). The outermost energy level is the sixth energy level. It has two electrons in the 6s sublevel.
It depends on the sublevel you refer to
The f sublevel has 7 orbitals, so it can contain up to 14 electrons.
sublevels s,p,d,and f
5 or 10
Energy levels are formed into sublevels which contain specific numbers of orbitals, each of which can contain two electrons with opposite spins. The s sublevel has 1 orbital, the p sublevel has 3 orbitals, the d sublevel has 5 orbitals, and the f sublevel has 7 orbitals.
Noble gases are very stable because their outermost electron shells contain the maximum number of electrons that those outermost shells can possess. This is a correct statement. Yes.
1: The outermost ring of hydrogen is the s-level, which can contain only two electrons, and a hydrogen atom itself already has one of these electrons.
The d sublevel always contains 5 orbitals. Therefore the d sublevel can accommodate 10 electrons just the same as 3d and 4d orbitals. Each of the 5 separate d orbitals can only contain two electrons.
According to the Octect Rule, an atom is most stable when its outermost shell has 8 electrons. So atoms try to attain 8 electrons in their outer shell.
transition metals b/c some, such has iron, have an incomplete 3d sublevel as well as a complete 4s level that are used in reactions
all other orbitals at that sublevel contain at least one electron (plato :P)
In the fifth period of the periodic table, the atoms of the elements in the first two groups are adding 1 and 2 electrons, respectively, to their highest energy 5s sublevel. Starting in group 3/IIIB and going through group 12/IIB, the atoms of those elements are adding electrons to their highest energy 4d sublevel. Since the d sublevel can contain a maxium of 10 electrons, there are 10 elements whose atoms are filling the 4d sublevel. Once the 4d sublevel is filled, the next higher energy sublevel is the 5p sublevel. Starting with the group 13/IIIA elements, the 5p sublevel is being filled. Since a p sublevel can contain a maximum of 6 electrons, there are six elements whose atoms are filling the 5p sublevel. 5s sublevel filling: 2 elements 4d sublevel filling: 10 elements 5p sublevel filling: 6 elements --------------------------------------- Total: 18 elements For a printable periodic table that includes electron configurations, go to the following link: http://www.nist.gov/pml/data/periodic.cfm
This atom gain the necessary number of electrons.
it would explode
protons, electrons and neutrons generally
S contains 2 P contains 6 D contains 10 F contains 14
The 2s is one orbital, it can contain up to two electrons, one spin up one spin down.
to fil the outermost energy level which is the level that contain all the valance electrons